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Given the following balanced chemical reaction: 4 NH3(g) 5 O2(g) --> 4 NO(g) 6H2O(L) Part A (2 points): Calculate the moles of H2O produced when 0.800 moles of NH3 react. The molar masses are not needed for this problem. Given the following balanced chemical reaction: Pb(s) PbO2(s) 2 H2SO4(aq) --> 2 PbSO4(s) 2 H2O(L) Molar masses needed for this problem (g/mol): PbSO4 = 303.3, PbO2 = 239.2, H2SO4 = 98.08 Part B (3 points): What mass of H2SO4 is needed to completely react with 50.5g of PbO2? Part C (3 points): Starting with the amount of H2SO4 in grams from Part B, how many grams of PbSO4 can be produced? Hint: your answer needs the same amount of sig figs as your answer in Part B.
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